Answer the following questions on a new wiki titled 15-1 Gas Notes Worksheet using the notes found at the bottom of the page.
Questions
Describe the position of particles in a gas.
Is a gas' shape definite? (will it keep a shape like a desk?)
Is a gas' volume definite? (will it stay in a 12 oz cup?)
Do gas' have higher or lower densities than a solid or a liquid?
What does compressible mean?
What does diffusion mean?
What does effusion mean?
What is the name of the theory that states that all matter is made of particles and that they are constantly moving?
Between solid, liquid, and gases, which particles move the least?
What is the name of this particle motion? (starts with a B)
Intermolecular forces attract molecules to each other. Kinetic energy causes particles to want to move away from each other. So which is stronger in a gas, the Kinetic energy or the intermolecular forces?
What is the measure of heat called?
What does a barometer measure?
How is a manometer different? (btw, Mr Bair rates a perfect 10 on most manometers)
Explain why pressure is sometimes measured in mm of mercury (mm Hg).
On a scale of 1-10, how aggrivating is it that there are 5 different units to measure the same thing? (760mm Hg = 760 torr = 101.3 kPa = 14.7 psi = 1 atm) (good news, you dont have to memorize these numbers... Ill tell em to ya, and so will the EOC)
Boyle, or crazy curly hair guy as I like to call him, compares pressure and volume with his equation. I will give you the equation on the test! So, solve this question if you dare.... But seriously do it. Its a part of your grade.
Using Boyle's Law:
The volume of the lungs is measured by the volume of air inhaled or exhaled. If the volume of the lungs is 2.400 L during exhalation and the pressure is 101.70 KPa, and the pressure during inhalation is 101.01 KPa, what is the volume of the lungs during inhalation?
Charles, or creepy stalker looking guy, compares Volume and Temperature with his equation. ... Solve the problem below
Using Charles' Law (You must always use KELVIN for Temperature because his beard is way cool (actually it is because his scale is a measure of energy.))
A sample of gas at 101.3kPa had a volume of 1.2L at 100K. What would its volume be at 273K at the same pressure?
Avogadro, (Im going to leave him alone. He looks like he had a tough life), compares number of moles and what other variable?
Define Dalton's law of partial pressures. If the pressure of oxygen gas collected over water is 750 mm Hg, and the pressure that the water vapor added was 22.4 mm Hg. What was the pressure of the oxygen gas?
How many moles of gas does it take to occupy 120 liters at a pressure of 2.3 atmospheres and a temperature of 340 K?
Using the same numbers from the previous question, what would happen to the temperature if the pressure increases to 3 atmospheres and everything else stayed the same?
Time Length
- 2 Days
InstructionsQuestions
- Describe the position of particles in a gas.
- Is a gas' shape definite? (will it keep a shape like a desk?)
- Is a gas' volume definite? (will it stay in a 12 oz cup?)
- Do gas' have higher or lower densities than a solid or a liquid?
- What does compressible mean?
- What does diffusion mean?
- What does effusion mean?
- What is the name of the theory that states that all matter is made of particles and that they are constantly moving?
- Between solid, liquid, and gases, which particles move the least?
- What is the name of this particle motion? (starts with a B)
- Intermolecular forces attract molecules to each other. Kinetic energy causes particles to want to move away from each other. So which is stronger in a gas, the Kinetic energy or the intermolecular forces?
- What is the measure of heat called?
- What does a barometer measure?
- How is a manometer different? (btw, Mr Bair rates a perfect 10 on most manometers)
- Explain why pressure is sometimes measured in mm of mercury (mm Hg).
- On a scale of 1-10, how aggrivating is it that there are 5 different units to measure the same thing? (760mm Hg = 760 torr = 101.3 kPa = 14.7 psi = 1 atm) (good news, you dont have to memorize these numbers... Ill tell em to ya, and so will the EOC)
- Boyle, or crazy curly hair guy as I like to call him, compares pressure and volume with his equation. I will give you the equation on the test! So, solve this question if you dare.... But seriously do it. Its a part of your grade.
- Using Boyle's Law:
- The volume of the lungs is measured by the volume of air inhaled or exhaled. If the volume of the lungs is 2.400 L during exhalation and the pressure is 101.70 KPa, and the pressure during inhalation is 101.01 KPa, what is the volume of the lungs during inhalation?
- Charles, or creepy stalker looking guy, compares Volume and Temperature with his equation. ... Solve the problem below
- Using Charles' Law (You must always use KELVIN for Temperature because his beard is way cool (actually it is because his scale is a measure of energy.))
- A sample of gas at 101.3kPa had a volume of 1.2L at 100K. What would its volume be at 273K at the same pressure?
- Avogadro, (Im going to leave him alone. He looks like he had a tough life), compares number of moles and what other variable?
- Define Dalton's law of partial pressures. If the pressure of oxygen gas collected over water is 750 mm Hg, and the pressure that the water vapor added was 22.4 mm Hg. What was the pressure of the oxygen gas?
- How many moles of gas does it take to occupy 120 liters at a pressure of 2.3 atmospheres and a temperature of 340 K?
- Using the same numbers from the previous question, what would happen to the temperature if the pressure increases to 3 atmospheres and everything else stayed the same?
Notes